The conductivity of $0.01 \ M$ aqueous acetic acid measured with a conductivity cell of cell constant $0.5 \ cm^{-1}$ at $298 \ K$ is $3.12 \times 10^{-4} \ S$. If the limiting molar conductivities of $H^{+}$ and $CH_3COO^{-}$ at the same temperature are $349$ and $41 \ S \ cm^2 \ mol^{-1}$ respectively,the dissociation constant of acetic acid is
- A$1.67 \times 10^{-4}$
- B$1.67 \times 10^{-5}$
- C$1.67 \times 10^{-3}$
- D$1.67 \times 10^{-6}$
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The number of incorrect statements from the following is:
$A.$ The electrical work that a reaction can perform at constant pressure and temperature is equal to the reaction Gibbs energy.
$B.$ $E_{cell}^0$ is dependent on the pressure.
$C.$ $\frac{dE_{cell}^0}{dT} = \frac{\Delta_{r}S^0}{nF}$.
$D.$ $A$ cell is operating reversibly if the cell potential is exactly balanced by an opposing source of potential difference.
$A.$ The electrical work that a reaction can perform at constant pressure and temperature is equal to the reaction Gibbs energy.
$B.$ $E_{cell}^0$ is dependent on the pressure.
$C.$ $\frac{dE_{cell}^0}{dT} = \frac{\Delta_{r}S^0}{nF}$.
$D.$ $A$ cell is operating reversibly if the cell potential is exactly balanced by an opposing source of potential difference.
DifficultJEE MAIN 2023
View SolutionThe molar conductance of $NaCl$,$HCl$,and $CH_{3}COONa$ at infinite dilution are $126.45$,$426.16$,and $91.0 \ S \ cm^{2} \ mol^{-1}$ respectively. The molar conductance of $CH_{3}COOH$ at infinite dilution is. Choose the right option for your answer. (In $S \ cm^{2} \ mol^{-1}$)
$A$ and $B$ are two metals. The standard reduction potentials of $A^{+}_{(aq)} / A_{(s)}$ and $B^{+}_{(aq)} / B_{(s)}$ are $-0.5 \ V$ and $+0.5 \ V$ respectively. What is the $\log K_C$ value for the following reaction at $298 \ K$?
$A_{(s)} + B^{+}_{(aq)} \rightleftharpoons A^{+}_{(aq)} + B_{(s)}$
(Given: $\frac{2.303 RT}{F} = 0.06 \ V$)
$A_{(s)} + B^{+}_{(aq)} \rightleftharpoons A^{+}_{(aq)} + B_{(s)}$
(Given: $\frac{2.303 RT}{F} = 0.06 \ V$)
The equilibrium constant of a $2$ electron redox reaction at $298 \, K$ is $3.8 \times 10^{-3}$. The cell potential $E^{\circ}$ (in $V$) and the free energy change $\Delta G^{\circ}$ (in $kJ \, mol^{-1}$) for this equilibrium,respectively are
MediumKVPY 2016
View SolutionMatch the column $I$ with column $II$ and mark the appropriate choice.
Column $I$ Column $II$ $A$. Kohlrausch law $i$. $\Lambda _{m}^o = \nu _+ \lambda _+^o + \nu _- \lambda _-^o$ $B$. Molar Conductivity $ii$. $\Lambda _m = \frac{\kappa \times 1000}{M}$ $C$. Degree of Dissociation $iii$. $\alpha = \frac{\Lambda _m}{\Lambda _m^o}$ $D$. Dissociation Constant $iv$. $K_a = \frac{C\alpha ^2}{1 - \alpha}$
| Column $I$ | Column $II$ |
|---|---|
| $A$. Kohlrausch law | $i$. $\Lambda _{m}^o = \nu _+ \lambda _+^o + \nu _- \lambda _-^o$ |
| $B$. Molar Conductivity | $ii$. $\Lambda _m = \frac{\kappa \times 1000}{M}$ |
| $C$. Degree of Dissociation | $iii$. $\alpha = \frac{\Lambda _m}{\Lambda _m^o}$ |
| $D$. Dissociation Constant | $iv$. $K_a = \frac{C\alpha ^2}{1 - \alpha}$ |
Medium
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